Q1-Q8 (1MARKS EACH)
Q9-Q18 (2MARKS EACH).
Q19-Q27 (3 MARKS EACH)
Q28-Q30 (5 MARKS EACH)
…………………………………………………………….. Q1. State law of constant composition.
Q2. Howe 0.5m of NaOH different from 0.5M ofNaOH?
Q3. State Heisenberg uncertainity principal.
Q4. Write general electronic configuration of d-block elements. Q5. Define Resonance.
Q6. What is compressibility factor?
Q7. Define Buffer solution? What is common ion effect?
Q8. What is Demineralised water?Q9. Calculate the concentration of nitric acid in moles per litre in a sample which has a density of 1.41g/ml and mass% of nitric acid is 69%. Q10. Calculate energy of one mole of photons of radiation whose frequency is 5x10raise to power 10 Hz.(page 39. Q.1) Q11. Write down the electronic configuration of copper and chromium. Q12. Calculate the wavelength of 100 gm of particle moving with a velocity of 100m/s. Q13. Complete the following:-

a) Na₂O+H₂0--
b) Cl₂07+H₂0-------
Q14:- Write resonance structure of NO₂ and SO3?Q15.:-What is electro negativity.How it is different from election gain enthalpy? Q16.on a ship sailing in pacific ocean where temp. is 23.4˚C a ballon is filled with 2L air what will be the volume of balloon when ship reaches Indian ocean where temp. is 26.1˚C?(page no.139) Q17.For the reaction

1.2Cl(g)----------Cl₂(g)What are the signs of ϪH and ϪS. 2.Define Enthalpy?
Q18. Calculate pH of 0.2MH₂SO4 solution?Q19.:- 1.An atomic orbital has n=3 What are the possible values of 1 and m? 2.List the quantum numbers(m and 1) of electrons for 3d orbital 3.Which of the following orbital’s are possible 1p,2s,2p and 3f Q20. 1.Write IUPAC name of element with atomic number 120.

2.Which of the following species will have layout and smallest size Mg,Mg²+,Al,Al3+ 3.Why cautions are smaller than anions in radii than their parent atoms? Q21.Discuss the shapes of following molecules on the basis of VSEPR model. 1.SiCl4 2. PH3 3.H₂0

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...chemical performance. The exact location of tellurium on the periodic table is group 16 period 5, to the right of the ladder that separates the metals and nonmetals. The international agreed code or chemical symbol for tellurium is Te, representing the first two letters of the name. The number of protons and electrons is 52, represented by the atomicnumber and the total mass of protons, electrons and neutrons in an atom is 127.60, which is represented by the atomic mass.
The boiling point for any element is when the temperature changes from a gas to liquid or liquid to gas. In comparison, the melting point for any element is when the temperature changes from liquid to a solid or solid to a liquid. For instance, Tellurium has a boiling point of 989.8 °C and a melting point of 449.5°C. As previously stated in the above paragraphs, the atomicnumber is a combination of the protons and electrons within the nucleus. The atomic mass, however, is the complete total of all the protons, electrons, and neutrons within the atom at rest. As shown on the periodic table, tellurium has an atomicnumber of 52, and a mass of 127.60. Isotopes are atoms with the same number of protons, but have different number of neutrons. Tellurium has 33 isotopes and when it occurs naturally it has a mix of eight isotopes: 120Te (0.1%),
122Te...

...﻿
Hybridization of AtomicOrbitals
Chemical bonding can either be ionic, covalent or metallic. In an ionic bond, there is a complete transfer of electrons such that one atom becomes positively charged or a cation and the other is negatively charged or an anion. Metallic bonding is a special type of ionic bonding but it involves only those transition metals. In covalent bonding, sharing of electrons is involved; the atomicorbitals share electrons to form the bond.
The localized electron model represents a molecule as a collection of atoms bound together by sharing electrons using their atomicorbitals. The Lewis structure represents the arrangement of the valence electrons of an atom. Upon drawing the Lewis structure, the molecular geometry or structure can be predicted according to the Valence Shell Electron Pair Repulsion Theory or VSEPR.
Atomicorbitals can combine to form hybrid orbitals. This is the process called hybridization. Hybridization can be sp3, sp2, or sp. The higher hybridizations involve the d orbitals which can form sp3d or sp3d2 hybridization.
Considering the methane molecule, CH4, the C and H are directly bonded. The valence shell of C has 2s and 2p while only 1s for H. In terms of the atomicorbitals, the 2p orbitals and 2s atomic...

...OxidationNumber
When elements combine to produce a compound, each element is assigned an “apparent” charge. This apparent charge, the charge an atom would have if both electrons in each bond were assigned to the more electronegative element, may be positive or negative. It is called the oxidationnumber or state of the element in the compound.
Oxidationnumbers are very useful in keeping track of what happens to electrons when various elements combine to form compounds. By remembering a few generalizations concerning oxidationnumbers, the correct chemical formulas for a large number of compounds can be written and it becomes unnecessary to memorize chemical formulas. The following rules will help to assign oxidation states:
I. Any element in its free state, meaning not combined with another element has an oxidationnumber of zero. Eg: Pb, C, O2, Ne has an oxidationnumber of zero.
II. The oxidationnumber of any monoatomic ion is equal to the charge on the ion. Here are some examples: Na2+ has a charge of +2, Fe3+ has a charge of +3, and Cl- has a charge of -1
III. Oxygen is assigned an oxidationnumber of -2, except in peroxides when it is -1. The oxidationnumber of...

...﻿The
Atomic and
Nuclear
Structure of
an Atom
The atom has three main components the protons, neutrons, and electrons. The protons and neutrons make up the nucleus, while the electrons are found outside the atom’s nucleus. Each component of an atom has a charge to it. The protons have a positive charge. The electrons have a negative charge, and the neutrons have a neutral charge.
The atoms also have a charge. For example hydrogen can be negative, positive or neutral. These are called ions. H would be a neutrally charged hydrogen atom, while H- would be a negatively charged hydrogen atom. H+ would be a positively charged hydrogen atom.
The structure of an atom can tell someone what type of atom it is. For example if an atom has one proton then it is a hydrogen atom. Also if it has one electron then it will have a proton, and if it has a hundred electrons then it will have a hundred protons. You cannot take away any of its protons, neutrons or electrons without changing the type of atom.
The atom is the smallest form of the elements. If we cut a piece of wood into its smallest form there would be an atom. The atom still has all of the characteristics of the original element, but it is much smaller. To best explain how small an atom is compare an atom to an apple, and the compare the apple to the Earth. The Earth is way bigger than the apple, and the apple is way bigger than the atom.
The atomicnumber is how we...

...&ATOMICNUMBER AND MASS NUMBERS
After reading this section you will be able to do the following:
* Define and determine the atomicnumber of an atom.
* Define and determine the mass number of an atom.
What is an atom's atomicnumber?
The number of protons in the nucleus of an atom determines an element's atomicnumber. In other words, each element has a unique number that identifies how many protons are in one atom of that element. For example, all hydrogen atoms, and only hydrogen atoms, contain one proton and have an atomicnumber of 1. All carbon atoms, and only carbon atoms, contain six protons and have an atomicnumber of 6. Oxygen atoms contain 8 protons and have an atomicnumber of 8. The atomicnumber of an element never changes, meaning that the number of protons in the nucleus of every atom in an element is always the same.
What is an atom's mass number?
All atoms have a mass number which is derived as follows.
Review:
1. An element's or isotope's atomicnumber tells how many protons are in its atoms.
2. An element's or isotope's mass number tells how many protons and neutrons in...

...﻿
YOUR NAME: Erin Alston, Kennedy Stuart, Amber Lamb and Stephonya Williams
EXPERIMENT TITLE: Oxidation: Cyclohexanone from Cyclohexanol by Hypochlorite Oxidation and Adipic Acid from Cyclohexanone
DATE: 4/18/2014
INTRODUCTION: In experiment 4, alcohol is oxidized to a ketone with household bleach. The product is then isolated by steam distillation and is extracted into the distillate with ether. After the removal of ether, it leaves the product cyclohexanone.
In experiment 6, cyclohexanone is oxidized by potassium permanganate. Manganese dioxide is filtered off and the filtrate is concentrated, acidified with hydrochloric acid and then cooled to yield crystalline adipic acid.
OBJECTIVE:
Experiment 4: To recover cyclohexanone from the oxidation of cyclohexanol by hypochlorite
Experiment 6: To recover adipic acid from the oxidation of cyclohexanone
CHEMICAL REAGENTS
Cyclohexanol
Acetic Acid
Chlorine (Bleach)
Thymol Blue (indicator)
Sodium Hydroxide
These reagents were all used during experiment 4.
APPARATUS USED
Simple distillation apparatus
250mL round bottomed flask
PROCEDURE: Experiment 4
8 mL of cyclohexanol was placed into a 250 mL Erlenmeyer flask, and then a thermometer was introduced to the cyclohexanol. A mixture of 4 mL of acetic acid and 115mL of commercial household bleach was slowly added to the flask, while swirling it. During adding the mixture, the temperature was kept between 40 degrees...

...Name:
Date of experiment: 04/02/12 Date of report: 04/03/12
Title: Oxidation – Reduction Activity Series
Purpose: To determine relative oxidizing and reducing strengths of a series of metals and ions. Oxidation and reduction reaction occur simultaneously side by side. A reduction reaction occurs only if an oxidation reaction occurs and vise-versa. Electrons are given in oxidation while in reduction electrons are gained. Oxidizing agent is a chemical substance which has a large tendency to gain electrons, while reducing agent is a chemical substance causes other substances to be reduced and itself oxidized. Procedure: For this lab was used metals and substances provided in the lab oxidation-reduction pack, and some extra materials. Using the well-plate and the correct amount of drops and the right metal on the right well, to see the reaction with each different substance. Observations: This experiment required some time and patience to analyze the results. For each well required a different substance and a different metal to be inserted in the well. Different metals react faster or slower depending the substance they are added. Na2SO3 with magnesium  bubbles appeared around the magnesium piece and we could predict a reaction. MgSO4 with zinc  No reaction observed Zn (NO3)2 with lead and aluminum  No reaction observed FeCl3 with lead and aluminum  reacts with foil, the piece dissolves in the...